Carlos is making phosphorus trichloride using the equation below. He uses 15.5 g of phosphorus and collects 50.9 g of phosphorus chloride. 2P +3Cl2 → 2PCl3 How much chlorine reacted with the phosphorus? 15.5 g 17.7 g 35.4 g 66.4 g

The mass of chlorine used in reaction has been 35.4 g. Thus, option C is correct.

The balanced chemical equation for the reaction has been:

From the balanced reaction, 2 moles of phosphorus forms, 2 moles of phosphorus chloride.

The moles of phosphorus used has been given as:

The moles of phosphorus in 15.5 grams has been:

The moles of phosphorus chloride in 50.9 grams has been:

Since, 2  moles of phosphorus forms 2 moles phosphorus chloride. From 0.50 moles phosphorus, 0.372 mol phosphorus chloride has been formed.

Thus, chloride has been the limiting reagent, and the moles of chloride used in reaction has been equivalent to phosphorus chloride formed.

The moles of chlorine used has been 0.558 mol. The mass of chlorine has been given as:

The mass of chlorine used in reaction has been 35.4 g. Thus, option C is correct.

For more information about mole, refer to the link:

link

35.4 g

Explanation:

The balanced reaction is :

To calculate the moles :

According to stoichiometry :

2 moles of phosphorous chloride are produced by = 3 moles of

Thus 0.37 moles of phosphorous chloride are produced by= of

Mass of

Thus 35.4 g of chlorine reacted with the phosphorus

yes it is balanced

the answer is the first option

explanation:

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